CsBr crystallises in a BCC lattice. The unit cell of length is 436.6pm given that the atomic mass of Cs is 133 amu and of Br is 80 amu and the density of CsBr is
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Answer:
The density of CsBr is .
Explanation:
Number of atom in unit cell = Z = 4
Density of CsBr = ?
Edge length of cubic unit cell= a
Atomic mass of Pt(M) = 195.08 g/mol
Formula used :
where,
= density
Z = number of atom in unit cell
M = Molar mass of compound
= Avogadro's number
a = edge length of unit cell
We have:
M =133 g/mol + 80 g/mol = 213 g/mol
1 pm =
Z = 2
On substituting all the given values , we will get the value of 'a'.
The density of CsBr is .
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